Question

A 3.0 l sample of helium gas is stored in a rigid, sealed container at 25 °c and 1.0 atm pressure. the temperature is increased to 125 °c. what is the new pressure of the gas?

Answer 1

To find the new pressure of the helium gas, use the combined gas law equation, which relates the initial and final pressure, volume, and temperature of the gas. Plug in the given values and solve for the final pressure. The final pressure of the gas can be calculated once the volume of the gas in the new container is known.

Step-by-step explanation:

To find the new pressure of the gas, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

Where P1 = initial pressure, V1 = initial volume, T1 = initial temperature, P2 = final pressure, V2 = final volume, and T2 = final temperature.

Substituting the given values, we have:
P1 = 1.0 atm, V1 = 3.0 L, T1 = 25 °C = 298 K
T2 = 125 °C = 398 K

Plugging these values into the equation, we can solve for P2:

P2 = (P1 * V1 * T2) / (V2 * T1)

P2 = (1.0 atm * 3.0 L * 398 K) / (V2 * 298 K)

The new pressure of the gas can be calculated once the volume of the gas in the new container is known.

Answer 2

Assume ideal gas for simplicity so we could use the ideal gas equation. The hint words in here are the 'rigid, sealed container'. It means the volume is constant. So, we will use Gay-Lussac's Law.

T₁/P₁ = T₂/P₂
We have to solve for P₂. The solution is as follows:

(25 + 273 K)/1 atm = (125 + 273 K)/P₂
Solving for P₂,
P₂ = 1.34 atm